Lesson Notes By Weeks and Term v4 - SHS 2
EQUILIBRIA
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EQUILIBRIA
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Subject: Chemistry
Class: SHS 2
Term: 2nd Term
Week: 3
Grade code: 2.1.2.LI.3
Strand code: 1
Sub-strand code: 2
Content standard code: 2.1.2.CS.2
Indicator code: 2.1.2.LI.3
Theme: PHYSICAL CHEMISTRY
Subtheme: EQUILIBRIA
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Welcome, learners! Today, we delve deeper into the world of acids and bases, a topic that affects us daily. Think about the sharp taste of lime juice for your *sobolo*, the acid in a car battery that helps start a vehicle, or the soap we use for washing. Not all acids and bases are the same; some are "strong" and others are "weak". Understanding this difference is crucial not just for passing examinations, but for safety in the lab and at home, for understanding biological processes in our bodies, and for many industrial applications in Ghana, from food processing to mining.
A. The Core Concept: Dissociation
The fundamental difference between strong and weak acids/bases is the extent to which they dissociate (or ionize) in water. Dissociation: The process where a compound splits into its constituent ions when dissolved in a solvent, like water.
Strong Acids & Bases: The "All-In" Dissociators
A strong acid is one that completely or fully dissociates in an aqueous solution. This means that nearly 100% of its molecules break apart to release hydrogen ions (H⁺). We represent this complete dissociation with a single forward arrow (→). Example (Strong Acid): Hydrochloric acid (HCl) ``` HCl(aq) → H⁺(aq) + Cl⁻(aq) ``` If you dissolve 1000 molecules of HCl in water, you will get approximately 1000 H⁺ ions and 1000 Cl⁻ ions. There will be virtually no undissociated HCl molecules left. *Common Examples:* HCl (Hydrochloric acid), H₂SO₄ (Sulphuric acid), HNO₃ (Nitric acid).